In the space of 1 liter, methane gas (ch4) is reacted with 6 moles of water vapor according to the reaction: if at equilibrium state is obtained 4 moles of hydrogen gas, how many moles of methane gas is needed for the equilibrium reaction?
the reaction is
CH4(g) + 2H2O(g) ----> CO2(g) + 4H2 (g)
Kc = 16 / 3
Kc = [CO2] [H2]^4 / [CH4] [H2O]^2
given :
equilibrium concentration
[H2] = 4 moles
so equilibrium concentration of CO2 must be 1 mole
equilibrium concentration of H2O = 6 - 2 = 4
putting values
16 /3 = [1] [4]^4 / [CH4] [4]^2
[CH4] = 0.333 moles
so moles of CH4 required = 1.33 moles
